1.1 Understand the arrangement, movement and energy of the particles in each of the three states of matter: solid, liquid and gas 1.2 Describe how the interconversion of solids, liquids and gases are achieved and recall the names used for these interconversions 1.3 Describe the changes in arrangement, movement and energy of particles during these interconversions
The Kinetic Particle Theory
The main ideas of the kinetic theory are (this is your factual knowledge)
All the matter consists of tiny particles; these particles can be atoms, molecules or ions.
All particular move and, therefore, have kinetic energy; they vibrate or move position or both
There are forces between the particles
When matter is heated its particles gain more kinetic energy and move faster or vibrate more
When matter is heated it expands as its particles move further apart
The temperature of a substance tells us the average amount of kinetic energy of all its particles
The Three States of Matter
We can use the kinetic theory to describe the three states of matter.
State
Forces of Attraction Between Particles
Energy of particles
Arrangement of particles
Movement/motion of particles
SOLID
Strong Forces
Little Energy
Particles are held in fixed positions making an ordered arrangement or lattice
Particles are close together
When heated they move slightly further apart form each other
Particles vibrate around a point
Particles cannot move from their positions
When heated they vibrate more and move further apart a little (expansion)
LIQUID
Forces of attraction have less effect so that particles still stick together
Moderate Energy
Particles are in a random/irregular arrangement
Particles are still fairly close together
When heated they move slightly further apart from each other
Particles can move past one another and move randomly
When heated they move faster and move further apart a little (expansion)
GAS
Forces of attraction have no effect - almost no forces holding them together
A lot of energy
Random arrangement
Particles are very far apart/a lot of space between them/large distance between them
When heated they move even further apart
Particles move randomly (each particle in its own direction) and very fast
Particles move freely, constantly and in straight lines
Particles bounce off the walls of the containers causing pressure
When heated the particles move faster and move much further apart (a lot of expansion)
Lets now use these ideas to explain the differences in physical properties between the three states of matter (application of knowledge)
OBSERVATIONS
EXPLANATION
SOLID
Solids have fixed shape and volume (volume depends on number of particles + space between them)
The particles are in a fixed position
Solids cannot be compressed
Solid atoms are already tight enough
Solids only expand a little when heated
Forces of attraction are too strong
LIQUID
Liquids have a fixed volume
Particles are quite close and attracted strength
Liquids do not have a fixed shape (depends on the position of the particles)
Particles can move past one another
Liquids can flow
Particles move rapidly and passes another particle
GAS
Gases do not have a fixed shape or volume
Gas particles can move freely
Gas can easily be compressed
They have large space between each particles
Gas always fill up available space
Particles can move freely
Changes in State of Matter
The heating graph below shows what happens to the state and temperature of a solid substance when it is heated.
The point where solid starts to become liquid is the melting point.
The point where liquid starts to become gas is the boiling point.
When a substance is heated its particles take in energy and use the energy to increase their movement and move further apart/ PARTICLES OR MOLECULES DO NOT GET BIGGER (OR SMALLER) when they are heated (or cooled).
Melting
When a solid is heated its particles gain energy and move faster. Eventually they gain enough energy to move away their positions and begin to vibrate around each other. The solid melts to form a liquid. The temperature at which solid melts is the melting point. The temperature at which a solid melts tells us how strongly its particles are held together. Substances with high melting points have strong forces of attraction between their particles. Substances with low melting points have weak forces between their particles.
Boiling
When a liquid is heated the particles gain energy and move around faster and faster. Some particles near the surface of the liquid have enough energy to escape into air and form vapor. This process is called evaporation. Eventually a temperature is reached at which the particles from the liquid surface so rapidly that bubbles of vapor (liquid) are formed.
Cooling Graphs (Energy is given out)
During the cooling, the particles lose energy, come closer together and when they collide, they stick together to form droplets forming a liquid
If cooled further in the liquid state, they eventually move so slowly that start vibrating around a point.
During condensing and freezing the particles lose energy as they need less energy because they slow down and come closer together again. The forces between the particles have a much greater effect.
1a: STATES OF MATTER
1.1 Understand the arrangement, movement and energy of the particles in each of the three states of matter: solid, liquid and gas
1.2 Describe how the interconversion of solids, liquids and gases are achieved and recall the names used for these interconversions
1.3 Describe the changes in arrangement, movement and energy of particles during these interconversions
The Kinetic Particle Theory
The main ideas of the kinetic theory are (this is your factual knowledge)
The Three States of Matter
We can use the kinetic theory to describe the three states of matter.
State
Forces of Attraction Between Particles
Energy of particles
Arrangement of particles
Movement/motion of particles
SOLID
LIQUID
GAS
Lets now use these ideas to explain the differences in physical properties between the three states of matter (application of knowledge)
OBSERVATIONS
EXPLANATION
Changes in State of Matter
The heating graph below shows what happens to the state and temperature of a solid substance when it is heated.
The point where solid starts to become liquid is the melting point.
The point where liquid starts to become gas is the boiling point.
When a substance is heated its particles take in energy and use the energy to increase their movement and move further apart/ PARTICLES OR MOLECULES DO NOT GET BIGGER (OR SMALLER) when they are heated (or cooled).
Melting
When a solid is heated its particles gain energy and move faster. Eventually they gain enough energy to move away their positions and begin to vibrate around each other. The solid melts to form a liquid. The temperature at which solid melts is the melting point. The temperature at which a solid melts tells us how strongly its particles are held together. Substances with high melting points have strong forces of attraction between their particles. Substances with low melting points have weak forces between their particles.
Boiling
When a liquid is heated the particles gain energy and move around faster and faster. Some particles near the surface of the liquid have enough energy to escape into air and form vapor. This process is called evaporation. Eventually a temperature is reached at which the particles from the liquid surface so rapidly that bubbles of vapor (liquid) are formed.
Cooling Graphs (Energy is given out)
During the cooling, the particles lose energy, come closer together and when they collide, they stick together to form droplets forming a liquid
If cooled further in the liquid state, they eventually move so slowly that start vibrating around a point.
During condensing and freezing the particles lose energy as they need less energy because they slow down and come closer together again. The forces between the particles have a much greater effect.
Changes of State